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Chapter 8: Problem 21

Name the following acids. Assume each compound is dissolved in water. \(\mathrm{HClO}_{2}\)

Short Answer

Expert verified
The acid name of \(\mathrm{HClO}_{2}\) when dissolved in water is chlorous acid.

Step by step solution

01

Identify the anion

First, we need to determine the anion in the given formula \(\mathrm{HClO}_{2}\). Here, the anion is \(\mathrm{ClO}_{2}^-\).
02

Name the anion

Next, we need to name the anion \(\mathrm{ClO}_{2}^-\). Since it has chlorine, it is called chlorite.
03

Name the acid

Finally, we have to name the acid. For anions ending in -ite, the corresponding acid has the suffix -ous. Therefore, the acid name of \(\mathrm{HClO}_{2}\) when dissolved in water is chlorous acid.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Anion Identification
Anions play a crucial role in forming acids. In chemistry, an anion is a negatively charged ion. When an acid is named, identifying the anion is the first step. To find the anion in a chemical compound, look for the part that gains electrons. For example, in \(\mathrm{HClO}_2 \), the anion is \(\mathrm{ClO}_2^-\). This is done by recognizing the corresponding negative ion that combines with hydrogen ions in the compound.
It is important because this anion will guide the naming of the acid. Here is a quick way to identify an anion:
  • Find the group of atoms left when you remove the hydrogen ions from the compound.
  • Determine its charge, which typically corresponds to a missing number of hydrogen atoms.
  • Recognize the group or the polyatomic ion it forms.
Mastering anion identification lays the foundation for understanding how substances interact to form different chemical compounds.
Acid Nomenclature
Once you've identified an anion, it's time to name the acid. Acid nomenclature is a method to systematically name acids, based on the anion they contain.
This is especially important when the acid is dissolved in water, as aqueous solutions have specific naming rules. The following tips can help in naming the acids:
  • If the anion ends in "-ate," the acid name will typically end in "-ic." For example, the sulfate anion \(\mathrm{SO}_4^{2-}\) leads to sulfuric acid \(\mathrm{H}_2\mathrm{SO}_4\).
  • If the anion ends in "-ite," the acid name will be "-ous." This is the case with the chlorite anion \(\mathrm{ClO}_2^-\), which becomes chlorous acid \(\mathrm{HClO}_2\).
This systematic approach simplifies the process of identifying acids and ensures clarity in communication about chemical substances.
Chemical Compounds in Water
When chemicals dissolve in water, they form aqueous solutions that behave differently than in other states. Acids are a common class of chemicals that we often encounter dissolved in water. Understanding how they interact in this state is key to mastering chemistry.
Here鈥檚 why water is important in naming acids:
  • When acids dissolve in water, they release hydrogen ions \( \mathrm{H}^+ \), which are crucial for the chemical's acidity.
  • The naming often follows the behavior of the compound in water, such as behaving as a strong or weak acid.
  • Anions derived from dissolved compounds help predict the formation of salts or gases during reactions.
Water鈥檚 role is pivotal because it influences properties like acidity and reactivity. Recognizing how acids change and adapt in aqueous solutions is important for fully grasping their chemical behavior.

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Most popular questions from this chapter

Compare and contrast the two covalent compounds identified by the names arsenic(III) oxide and diarsenic trioxide.

State the steps used to draw Lewis structures.

Draw the Lewis structure for a molecule of each of these compounds and ions. \(\begin{array}{ll}{\text { a. } \mathrm{H}_{2} \mathrm{S}} & {\text { c. } \mathrm{SO}_{2}} \\ {\text { b. } \mathrm{BF}_{4}-} & {\text { d. } \mathrm{SeCl}_{2}}\end{array}\)

Draw the Lewis structure for BH_ \(_{3}\)

State the molecular formula for each compound listed below. \(\begin{array}{ll}{\text { a. dinitrogen trioxide }} & {\text { d. chloric acid }} \\ {\text { b. nitrogen monoxide }} & {\text { e. sulfuric acid }} \\\ {\text { c. hydrochloric acid }} & {\text { f. sulfurous acid }}\end{array}\)
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